The degree of dissociation of 0.1 M acid HA | vedclass

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(C) The degree of dissociation $\alpha$ for a weak acid is related to the dissociation constant $K_a$ and concentration $C$ by the formula: $\alpha =

Vedclass · Accepted Answer

$2.5 	imes 10^{-4}$

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(C) The degree of dissociation $\alpha$ for a weak acid is related to the dissociation constant $K_a$ and concentration $C$ by the formula: $\alpha = \sqrt{\frac{K_a}{C}}$.Given: $C = 0.1 \ M$ and $\alpha = 5 \% = 0.05$.Rearranging the formula for $K_a$ (or $K_c$ for the acid dissociation equilibrium): $K_a = \alpha^2 	imes C$.Substituting the values: $K_a = (0.05)^2 	imes 0.1$.$K_a = 0.0025 	imes 0.1 = 0.00025 = 2.5 	imes 10^{-4}$.Thus, the value of $K_c$ is $2.5 	imes 10^{-4}$.

The degree of dissociation of $0.1 \ M$ acid $HA$ is $5 \%$. The value of $K_c$ of $HA$ is

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